Nitric acid 70% has a specific gravity of 1.42. find the normality and molarity of the acid
kvnmurty:
HNO3 acid solution has specific gravity of 1.42g/ml and contains 70% by strength HNO3. Calculate a)Normality Of Acid b)Volume of acid that contains 63g pure acid c)Volume of water required to make 1N solution from 2ml concentrated HNO3
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Nitric acid H NO3: molecular mass = 63
mixture 70% by mass ...
70gm HNO3 mixed with 30gm (=30 ml) of water to get 100 gm of acid soln
Density 1.42 gm/cm^3
=> volume of 100 gm solution is = 100 /1.42 = 70.422 cm^3
So in 70.422 cm^3 we have 70gm of HNO3 ie., 70/63 moles.
Molarity = 70/63 * 1000/70.422 = 15.78 M
Normality = 15.78 N same as Molarity ,
as one mole of H NO3 gives rise to only one mole of H+ ions.
mixture 70% by mass ...
70gm HNO3 mixed with 30gm (=30 ml) of water to get 100 gm of acid soln
Density 1.42 gm/cm^3
=> volume of 100 gm solution is = 100 /1.42 = 70.422 cm^3
So in 70.422 cm^3 we have 70gm of HNO3 ie., 70/63 moles.
Molarity = 70/63 * 1000/70.422 = 15.78 M
Normality = 15.78 N same as Molarity ,
as one mole of H NO3 gives rise to only one mole of H+ ions.
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1
Answer:
molarity is 15.8 molar
hope it will help u
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